First slide

Faraday's Laws

Question

What is the approximate quantity of electricity in coulombs required to deposit all the silver from 500 ml 1M AgNO₃ aqueous solution ? (At. wt. of Ag = 108)

Moderate

A

96500
B

24125
C

48250
D

12062.5

Solution

No. of eq. of Ag deposited = vol(lit) x M x valency=0.5 x 1 x 1 =0.5
$i \times t (Coulombs) = 96500 \times eq of Ag deposited = 96500 \times 0.5 = 48250$

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